Gold metal is extracted from its ore by treating the crushed rock with an aerated cyanide solution. The unbalanced equation for the reaction is {Au}( {s})+ {CN}^{-}( {aq})+ {O}_{2}( {g}) \to {Au}( {CN})_{2}^{-}( {aq}) Use any of the following data at 27^{\circ} {C} to calculate ∆ {G} ' for this reaction in basic solution. Given {K}_{f} for {Au}( {CN})_{2}^{-}=10^{98} {O}_{2}( {g})+4 {H}^{+}( {aq})+4 {e}^{-} \to 2 {H}_{2} {O}(ℓ) {E}^{*}=1.2 {V} {Au}^{3+}( {aq})+3 {e}^{-} \to {Au}( {s}) E=1.5 {V} Use equation ∆ G^{' '}=-2 R T \log _{10} Q and R=8 {Jmol}^{-1} {K}^{-1}, F=96500 {C}. Give your answer (magnitude only) in {kJ}.

JEE Advanced 2020 Concept Recapitulation Test 4 Paper 1

Question : 32 of 54

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Gold metal is extracted from its ore by treating the crushed rock with an aerated cyanide solution. The unbalanced equation for the reaction is Au(s)+CN−(aq)+O2(g)→Au(CN)2−(aq) Use any of the following data at 27∘C to calculate ∆G ' for this reaction in basic solution. Given Kf for Au(CN)2−=1098 O2(g)+4H+(aq)+4e−→2H2O(ℓ)‌‌E*=1.2V Au3+(aq)+3e−→Au(s) E=1.5V Use equation ∆G′′=−2RTlog10Q and R=8Jmol−1K−1,F=96500C. Give your answer (magnitude only) in kJ.

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